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Chemistry > Atomic Theory > Flashcards

Atomic Theory Flashcards

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1
Q

Define radioactivity.

A

Radioactivity is the spontaneous breaking up of an unstable nucleas with the emission of one or more types of radiation.

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2
Q

Explain Heisenberg’s uncertainty principle.

A

The more closely you are to knowing the position of an electron the further you are from knowing it’s velocity.

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3
Q

Electronegativity down a group.

A

~Shielding effect

~Bigger atomic radius

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4
Q

Electronegativity across a group

A

~Increases
~Increase in nuclear charge
~Smaller atomic radius

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5
Q

Define half life.

A

Time taken for half of the nuclei in a sample to decay.

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6
Q

What’s atomic mass?

A

Number of protons in the nucleas of an atom.

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7
Q

The trend in electronegativity values down the first group of elements.

A

EN vales decrease down group because of shielding effect.

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8
Q

Define orbitals

A

Region in the space around the nucleas of an atom which electrons are most likely to be found.

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9
Q

Relative atomic mass

A

The average mass of an element as it occurs in nature compared to 1/12 of the mass of a 12 carbon isotope.

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10
Q

What is electronegativity?

A

Measure of attractiveness an atom has for a shared pair of electrons in a covalent bond.

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11
Q

What is the first ionisation energy?

A

Minimum energy required to remove the most loosely bound electron form an atom in its ground state.

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12
Q

What is molar mass?

A

The mass in grams of a mole of that substance.

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13
Q

What is atomic radius ?

A

Half the distance between the nuclei of two singly covalenty bonded atoms./ of two identical atoms joined by a single covalent bond

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14
Q

What is mass number?

A

Number of protons+ neutrons

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15
Q

Define isotopes

A

Atoms of the same element which have same number of protons but different numbers of neutrons.

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16
Q

What was the purpose of Milikan’s oil drop experiment?

A

To determine the charge of an electron

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17
Q

Name the scientist who identified cathode rays as a subatomic particle and also measure the charge to mass ratio?

A

J. J. Thompson

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18
Q

Describe Thompson’s “plum pudding”

A

model of the atom which had negatively-charged electrons embedded within a positively-charged “soup”/ sphere

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19
Q

Rutherford used alpha particles. What are these?

A

Helium nucleus. Two protons and two neutrons

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20
Q

2 properties of cathode rays

A

Travel in straight lines/ negligible mass/ negatively charged

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21
Q

State two assumptions of Dalton’s atomic theory of 1808

A

Atoms are small and indivisible

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22
Q

Who measured the charge of the electron?

A

Millikan

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23
Q

Who measured the ratio of charge to mass of an electron

A

J. J. Thompson

24
Q

What did Rutherford do?

A

Proved that electrons in an atom reside in an electron cloud surrounding a small dense positive nucleus

25
Q

Law of conservation of mass

A

When a chemical reaction takes place, matter is neither created or destroyed but merely changes from one form to another.

26
Q

Matter

A

Anything that occupies space and has mass.

27
Q

Relative molecular mass

A

Sum of relative atomic masses of all atoms in a molecule of the compound compared to 1/12 of the mass of a carbon-12 isotope

28
Q

Three fundamental processes that occurred in the mass spectrometer

A

Ionisation/ acceleration/ separation

29
Q

What result did Rutherford expect to get when thin gold foil was bombarded with alpha particles?

A

Alpha particles were expected to pass straight through/ Un deflected

30
Q

How did the actual result of Rutherford’s experiment differ from the expected result

A

Some particles were deflected at large angles /nuclease positive / almost all passed through/ some bounced straight back

31
Q

How was the model of atomic changed as a result of Rutherford’s experiment

A

Large electron cloud surrounding/ atoms mostly empty space/ nuclease very small

32
Q

Energy level

A

Shell which electrons of equal energy can occupy

33
Q

Aufbau principle

A

Electrons occupy the lowest available energy level

34
Q

What was Dalton’s atomic theory

A

Matter composed of atoms/ atoms are tiny particles/ atoms are indivisible/ cannot be created or destroyed

35
Q

What happens in a radioactive nuclease during beta decay?

A

Neutron changes into proton and an electron which is emitted

36
Q

How did Mendeleev arrange the elements in the periodic table of 1869?

A

According to atomic weight/ in groups of similarities properties

37
Q

How do we know that any new element discovered in the future will be super heavy

A

No gaps in modern periodic table/ all other lighter elements known

38
Q

Main energy levels in electron transition that gives rise to the first line of the balmer series in the emission spectrum of the hydrogen atom

A

3 and 2

39
Q

Describe trend in covalent radii for atoms of the second period of the periodic table

A

Increases because of additional shells/ increase in nuclear charge

40
Q

Term used for the condition of the hydrogen atom when its electron occupies any of the levels E2,E3,etc?

A

Excited state

41
Q

What causes the electron to leave the E1 level?

A

Acquires energy /heat

42
Q

Why does the electron not remain in any of the levels E2,E3,etc?

A

Higher energy states unstable

43
Q

How does modern atomic theory describe the behaviour of electrons?

A

Electrons have both wave and particle properties

44
Q

Cathode rays

A

Beams of electrons/ negatively charged

45
Q

Advantage of arranging elements in order of atomic number

A

Indicates gaps/ undiscovered elements / tellurium and iodine positions are justified

46
Q

Position of tellurium and iodine in the 1869 table

A

Listed according to chemical properties/ listing by atomic mass wouldn’t group them with elements of the similar properties

47
Q

Periodic system in context of Mendeleev’s 1869 table

A

Elements listed according to atomic mass/ properties repeat periodically

48
Q

Why the elements of group 18 in the table are chemically inert

A

Stable arrangement of electrons/ do not lose or gain electrons

49
Q

Scientist who discovered presence of cathode rays

A

Crookes( paddle wheel experiments)

50
Q

Who discovered the neutron?

A

Chadwick

51
Q

Give a reason for the general increase in first ionisation energy across a period of the periodic table

A

the increase in nuclear charge having a greater pull on the electrons and therefore more energy is required to remove electrons

52
Q

Explain why the general increase in first IE is interuppted

A

The repulsion between 2 electrons makes one of them easier to remove/ beacuse boron has a smaller value than baylium

53
Q

Mass spectrometer processes

A
  1. Vaporitasion
  2. Ionisation
  3. Acceleration
  4. Seperation
  5. Detection
  6. Display
54
Q

Describe ionisation process in mass spectrometer

A

The sample is ionised by bombarding it with high energy electrons

55
Q

Describe acceleration and sepearation in mass soectrometer (process 3&4)

A

Acceleartion: positive ions are accelerated by negatively charged plates.
Seperation: ions are deflected by magnetic feild

56
Q

What is the last process in mass spectometer

A

Detection: ions are detected by a sensitive plate

57
Q

What are gamma particles?

A

Electromagnetic radiation. Highly penetrating

Chemistry (19 decks)

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